Given: Hg2+(aq)+ 2e- Hg(s); E° = 0.85 V Li+(aq)+ e- Li(s); E° = -3.04 V Br2(l)+ 2e- 2Br-(aq); E° = 1.07 V Au+(aq)+ e- Au(s); E° = 1.69 V Cl2(g)+ 2e- 2Cl-(aq); E° = 1.36 V Which of the following species is the best reducing agent?

A) Hg B) Li+ C) Au D) Cl- E) Br- A) Hg B) Li+ C) Au D) Cl- E) Br-

A zinc-copper voltaic cell is represented as follows: Zn(s)| Zn2+(1.0 M)|| Cu2+(1.0 M)| Cu(s) Which of the following statements is false?

A) The copper electrode is the anode. B) Reduction occurs at the copper electrode during discharge. C) The mass of the zinc electrode decreases during discharge. D) Electrons flow through the external circuit from the zinc electrode to the copper electrode. E) The concentration of Cu2+ decreases during discharge. A) The copper electrode is the anode. B) Reduction occurs at the copper electrode during discharge. C) The mass of the zinc electrode decreases during discharge. D) Electrons flow through the external circuit from the zinc electrode to the copper electrode. E) The concentration of Cu2+ decreases during discharge.

The electrochemical reaction which powers a lead-acid storage battery is as follows: Pb(s)+ PbO2(s)+ 4H+(aq)+ 2SO42-(aq)→ 2PbSO4(s)+ 2H2O(l) A single cell of this battery consists of a Pb electrode and a PbO2 electrode,each submerged in sulfuric acid.What reaction occurs at the cathode during discharge?

A) Pb(s)is reduced to PbSO4(s). B) PbO2(s)is reduced to PbSO4(s). C) PbO2(s)is oxidized to PbSO4(s). D) Pb(s)is oxidized to PbSO4(s). E) H+ is oxidized to H2O(l). A) Pb(s)is reduced to PbSO4(s). B) PbO2(s)is reduced to PbSO4(s). C) PbO2(s)is oxidized to PbSO4(s). D) Pb(s)is oxidized to PbSO4(s). E) H+ is oxidized to H2O(l).

Given: Zn2+(aq)+ 2e- Zn(s); E° = -0.76 V Cr3+(aq)+ 3e- Cr(s); E° = -0.74 V Fe2+(aq)+ 2e- Fe(s); E° = -0.41 V Cd2+(aq)+ 2e- Cd(s); E° = -0.40 V Sn2+(aq)+ 2e- Sn(s); E° = -0.15 V Hg2+(aq)+ 2e- Hg(s); E° = 0.85 V Au+(aq)+ e- Au(s); E° = 1.69 V Under standard-state conditions,which of the following metals will reduce Hg2+ to Hg but will not reduce Cd2+ to Cd?

A) Cr B) Zn C) Fe D) Sn E) Au A) Cr B) Zn C) Fe D) Sn E) Au

In the electrolysis of an acid solution,oxygen can be produced by the following half-reaction: 2H2O(l)→ O2(g)+ 4H+(aq)+ 4e- How many moles of O2 can be produced from a solution that was electrolyzed for 6.50 h using a current of 5.40 A?

A) 2.03 × 108 mol B) 3.05 × 109 mol C) 9.09 × 10-5 mol D) 0.327 mol E) 1.3 mol A) 2.03 × 108 mol B) 3.05 × 109 mol C) 9.09 × 10-5 mol D) 0.327 mol E) 1.3 mol

How many faradays are required to convert a mole of NO3- ions to NH4+ ions?

A) 4 B) 7 C) 8 D) 6 E) 5 A) 4 B) 7 C) 8 D) 6 E) 5

Consider the following standard reduction potentials: Mg2+(aq)+ 2e- Mg(s); E° = -2.38 V V2+(aq)+ 2e- V(s); E° = -1.18 V Cu2+(aq)+ e- Cu+(aq); E° = 0.15 V Which of the following reactions will proceed spontaneously from left to right under standard-state conditions?

A) Mg(s)+ 2Cu2+(aq)→ Mg2+(aq)+ 2Cu+(aq) B) V2+(aq)+ 2Cu+(aq)→ V(s)+ 2Cu2+(aq) C) Mg2+(aq)+ 2Cu+(aq)→ 2Cu2+(aq)+ Mg(s) D) Mg2+(aq)+ V(s)→ V2+(aq)+ Mg(s) E) 2Cu2+(aq)+ 2Cu+(aq)→ Mg2+(aq)+ Mg(s) A) Mg(s)+ 2Cu2+(aq)→ Mg2+(aq)+ 2Cu+(aq) B) V2+(aq)+ 2Cu+(aq)→ V(s)+ 2Cu2+(aq) C) Mg2+(aq)+ 2Cu+(aq)→ 2Cu2+(aq)+ Mg(s) D) Mg2+(aq)+ V(s)→ V2+(aq)+ Mg(s) E) 2Cu2+(aq)+ 2Cu+(aq)→ Mg2+(aq)+ Mg(s)

Exam 19: Electrochemistry

A strip of iron is placed in a 1 M solution of iron(II)sulfate,and a strip of copper is placed in a 1 M solution of copper(II)chloride.The two solutions are connected with a salt bridge,and the two metals are connected by a wire. Reduction Half-Reaction E° (V) Fe²⁺(aq)+ 2e^- Fe(s) -0)41Cu²⁺(aq)+ 2e^- Cu(s) 0)34 Which of the following takes place?

(Multiple Choice)

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Question 41

Given: Hg²⁺(aq)+ 2e^- Hg(s); E° = 0.85 V Li⁺(aq)+ e^- Li(s); E° = -3.04 V Br₂(l)+ 2e^- 2Br^-(aq); E° = 1.07 V Au⁺(aq)+ e^- Au(s); E° = 1.69 V Cl₂(g)+ 2e^- 2Cl^-(aq); E° = 1.36 V Which of the following species is the best reducing agent?

(Multiple Choice)

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Question 42

When the following oxidation-reduction reaction in acidic solution is balanced,what is the lowest whole-number coefficient for H⁺,and on which side of the balanced equation should it appear? MnO₄^-(aq)+ I^-(aq)→ Mn²⁺(aq)+ I₂(s)

(Multiple Choice)

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Question 43

What is the value of the reaction quotient,Q,for the voltaic cell constructed from the following two half-reactions when the Zn²⁺ concentration is 0.0120 M and the Ag⁺ concentration is 1.27 M?

(Multiple Choice)

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Question 44

A cell consists of a magnesium electrode immersed in a solution of magnesium chloride and a silver electrode immersed in a solution of silver nitrate.The two half-cells are connected by means of a salt bridge.It is possible to increase the voltage of the cell by

(Multiple Choice)

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Question 45

For the cell reaction 2MnO₄^- (aq)+ 5SO₂(g)+ 2H₂O(l) → 2Mn²⁺(aq)+ 5SO^2-₄ (aq)+ 4H⁺(aq) The standard cell potential is 1.34 V.To determine the cell potential at nonstandard conditions,what is the value that should be used for n in the Nernst equation?

(Multiple Choice)

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Question 46

A zinc-copper voltaic cell is represented as follows: Zn(s)| Zn²⁺(1.0 M)|| Cu²⁺(1.0 M)| Cu(s) Which of the following statements is false?

(Multiple Choice)

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Question 47

The electrochemical reaction which powers a lead-acid storage battery is as follows: Pb(s)+ PbO₂(s)+ 4H⁺(aq)+ 2SO₄^2-(aq)→ 2PbSO₄(s)+ 2H₂O(l) A single cell of this battery consists of a Pb electrode and a PbO₂ electrode,each submerged in sulfuric acid.What reaction occurs at the cathode during discharge?

(Multiple Choice)

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Question 48

Given: Pb²⁺ (aq)+ 2e¯ Pb(s); Eº = -0.13V What is the standard Gibbs free-energy change for the following reaction? 2Cr(s)+ 3Pb²⁺ (aq)→ 3Pb(s)+ 2Cr³⁺ (aq)

(Multiple Choice)

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Question 49

Electrolysis of a molten salt with the formula MCl,using a current of 3.86 A for 16.2 min,deposits 1.52 g of metal.Identify the metal.(1 faraday = 96,485 coulombs)

(Multiple Choice)

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Question 50

Given: Zn²⁺(aq)+ 2e^- Zn(s); E° = -0.76 V Cr³⁺(aq)+ 3e^- Cr(s); E° = -0.74 V Fe²⁺(aq)+ 2e^- Fe(s); E° = -0.41 V Cd²⁺(aq)+ 2e^- Cd(s); E° = -0.40 V Sn²⁺(aq)+ 2e^- Sn(s); E° = -0.15 V Hg²⁺(aq)+ 2e^- Hg(s); E° = 0.85 V Au⁺(aq)+ e^- Au(s); E° = 1.69 V Under standard-state conditions,which of the following metals will reduce Hg²⁺ to Hg but will not reduce Cd²⁺ to Cd?

(Multiple Choice)

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Question 51

In the electrolysis of an acid solution,oxygen can be produced by the following half-reaction: 2H₂O(l)→ O₂(g)+ 4H⁺(aq)+ 4e^- How many moles of O₂ can be produced from a solution that was electrolyzed for 6.50 h using a current of 5.40 A?

(Multiple Choice)

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Question 52

If the cell is initially at standard-state conditions,which of the following statements is true? Zn²⁺(aq)+ 2e^- Zn(s); E° = -0.76 V Cu²⁺(aq)+ 2e^- Cu(s); E° = 0.34 V

(Multiple Choice)

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Question 53

How many faradays are required to convert a mole of NO₃^- ions to NH₄⁺ ions?

(Multiple Choice)

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Question 54

Consider the following standard reduction potentials: Mg²⁺(aq)+ 2e^- Mg(s); E° = -2.38 V V²⁺(aq)+ 2e^- V(s); E° = -1.18 V Cu²⁺(aq)+ e^- Cu⁺(aq); E° = 0.15 V Which of the following reactions will proceed spontaneously from left to right under standard-state conditions?

(Multiple Choice)

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Question 55

The anode in a voltaic cell and in an electrolytic cell is

(Multiple Choice)

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Question 56

A current of 13.0 A is passed through molten magnesium chloride for 16.0 h.How many moles of magnesium metal could be produced via this electrolysis?

(Multiple Choice)

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Question 57

Balance the following half-reaction occurring in basic solution. MnO₂(s)→ Mn(OH)₂(s)

(Multiple Choice)

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Question 58

The cell potential of the following cell is determined using an unspecified concentration of acid.What is the pH of the acid solution given that the measured cell potential is -0.508 V and the anode reduction potential (E°)is 0.222 V at 25°C? Ag(s)| AgCl(s)| Cl−(1.0 M)|| H⁺(aq,? M)| H₂(g,1.0 atm)| Pt(s)

(Multiple Choice)

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Question 59

When an aqueous solution of sodium sulfate is electrolyzed,what are the expected products? Reduction Half-Reaction E° (V) Na⁺(aq)+ e¯ Na(s) -2.71 2H₂O(l)+ 2e^- H₂(g)+ 2OH^-(aq) -0.83 2H⁺(aq)+ 2e^- H₂(g) 0.00 O₂(g)+ 4H⁺(aq)+ 4e^- 2H₂O(l)1.23 S₂O₈^2-(aq)+ 2e^- 2SO₄^2-(aq) 2.01

(Multiple Choice)

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Question 60

Showing 41 - 60 of 122

Given: Hg²⁺(aq)+ 2e^- Hg(s); E° = 0.85 V Li⁺(aq)+ e^- Li(s); E° = -3.04 V Br₂(l)+ 2e^- 2Br^-(aq); E° = 1.07 V Au⁺(aq)+ e^- Au(s); E° = 1.69 V Cl₂(g)+ 2e^- 2Cl^-(aq); E° = 1.36 V Which of the following species is the best reducing agent?

When the following oxidation-reduction reaction in acidic solution is balanced,what is the lowest whole-number coefficient for H⁺,and on which side of the balanced equation should it appear? MnO₄^-(aq)+ I^-(aq)→ Mn²⁺(aq)+ I₂(s)

What is the value of the reaction quotient,Q,for the voltaic cell constructed from the following two half-reactions when the Zn²⁺ concentration is 0.0120 M and the Ag⁺ concentration is 1.27 M?

A cell consists of a magnesium electrode immersed in a solution of magnesium chloride and a silver electrode immersed in a solution of silver nitrate.The two half-cells are connected by means of a salt bridge.It is possible to increase the voltage of the cell by

For the cell reaction 2MnO₄^- (aq)+ 5SO₂(g)+ 2H₂O(l) → 2Mn²⁺(aq)+ 5SO^2-₄ (aq)+ 4H⁺(aq) The standard cell potential is 1.34 V.To determine the cell potential at nonstandard conditions,what is the value that should be used for n in the Nernst equation?

A zinc-copper voltaic cell is represented as follows: Zn(s)| Zn²⁺(1.0 M)|| Cu²⁺(1.0 M)| Cu(s) Which of the following statements is false?

Given: Pb²⁺ (aq)+ 2e¯ Pb(s); Eº = -0.13V What is the standard Gibbs free-energy change for the following reaction? 2Cr(s)+ 3Pb²⁺ (aq)→ 3Pb(s)+ 2Cr³⁺ (aq)

Electrolysis of a molten salt with the formula MCl,using a current of 3.86 A for 16.2 min,deposits 1.52 g of metal.Identify the metal.(1 faraday = 96,485 coulombs)

In the electrolysis of an acid solution,oxygen can be produced by the following half-reaction: 2H₂O(l)→ O₂(g)+ 4H⁺(aq)+ 4e^- How many moles of O₂ can be produced from a solution that was electrolyzed for 6.50 h using a current of 5.40 A?

If the cell is initially at standard-state conditions,which of the following statements is true? Zn²⁺(aq)+ 2e^- Zn(s); E° = -0.76 V Cu²⁺(aq)+ 2e^- Cu(s); E° = 0.34 V

How many faradays are required to convert a mole of NO₃^- ions to NH₄⁺ ions?

Consider the following standard reduction potentials: Mg²⁺(aq)+ 2e^- Mg(s); E° = -2.38 V V²⁺(aq)+ 2e^- V(s); E° = -1.18 V Cu²⁺(aq)+ e^- Cu⁺(aq); E° = 0.15 V Which of the following reactions will proceed spontaneously from left to right under standard-state conditions?

The anode in a voltaic cell and in an electrolytic cell is

A current of 13.0 A is passed through molten magnesium chloride for 16.0 h.How many moles of magnesium metal could be produced via this electrolysis?

Balance the following half-reaction occurring in basic solution. MnO₂(s)→ Mn(OH)₂(s)

When an aqueous solution of sodium sulfate is electrolyzed,what are the expected products? Reduction Half-Reaction E° (V) Na⁺(aq)+ e¯ Na(s) -2.71 2H₂O(l)+ 2e^- H₂(g)+ 2OH^-(aq) -0.83 2H⁺(aq)+ 2e^- H₂(g) 0.00 O₂(g)+ 4H⁺(aq)+ 4e^- 2H₂O(l)1.23 S₂O₈^2-(aq)+ 2e^- 2SO₄^2-(aq) 2.01

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Exam 19: Electrochemistry

Given: Hg2+(aq)+ 2e- Hg(s); E° = 0.85 V Li+(aq)+ e- Li(s); E° = -3.04 V Br2(l)+ 2e- 2Br-(aq); E° = 1.07 V Au+(aq)+ e- Au(s); E° = 1.69 V Cl2(g)+ 2e- 2Cl-(aq); E° = 1.36 V Which of the following species is the best reducing agent?

When the following oxidation-reduction reaction in acidic solution is balanced,what is the lowest whole-number coefficient for H+,and on which side of the balanced equation should it appear? MnO4-(aq)+ I-(aq)→ Mn2+(aq)+ I2(s)

What is the value of the reaction quotient,Q,for the voltaic cell constructed from the following two half-reactions when the Zn2+ concentration is 0.0120 M and the Ag+ concentration is 1.27 M?

A cell consists of a magnesium electrode immersed in a solution of magnesium chloride and a silver electrode immersed in a solution of silver nitrate.The two half-cells are connected by means of a salt bridge.It is possible to increase the voltage of the cell by

For the cell reaction 2MnO4- (​aq​)+ 5SO2(g)+ 2H2O(l) → 2Mn2+(aq)+ 5SO2-4 (aq​)+ 4H+(aq) The standard cell potential is 1.34 V.To determine the cell potential at nonstandard conditions,what is the value that should be used for n in the Nernst equation?

A zinc-copper voltaic cell is represented as follows: Zn(s)| Zn2+(1.0 M)|| Cu2+(1.0 M)| Cu(s) Which of the following statements is false?

Given: Pb2+ (aq​)+ 2e¯ Pb(​s​); ​E​º = -0.13V What is the standard Gibbs free-energy change for the following reaction? 2Cr(​s​)+ 3Pb2+ (aq​)→ 3Pb(​s​)+ 2Cr3+ (aq)

Electrolysis of a molten salt with the formula MCl,using a current of 3.86 A for 16.2 min,deposits 1.52 g of metal.Identify the metal.(1 faraday = 96,485 coulombs)

In the electrolysis of an acid solution,oxygen can be produced by the following half-reaction: 2H2O(l)→ O2(g)+ 4H+(aq)+ 4e- How many moles of O2 can be produced from a solution that was electrolyzed for 6.50 h using a current of 5.40 A?

If the cell is initially at standard-state conditions,which of the following statements is true? Zn2+(aq)+ 2e- Zn(s); E° = -0.76 V Cu2+(aq)+ 2e- Cu(s); E° = 0.34 V

How many faradays are required to convert a mole of NO3- ions to NH4+ ions?

Consider the following standard reduction potentials: Mg2+(aq)+ 2e- Mg(s); E° = -2.38 V V2+(aq)+ 2e- V(s); E° = -1.18 V Cu2+(aq)+ e- Cu+(aq); E° = 0.15 V Which of the following reactions will proceed spontaneously from left to right under standard-state conditions?

The anode in a voltaic cell and in an electrolytic cell is

A current of 13.0 A is passed through molten magnesium chloride for 16.0 h.How many moles of magnesium metal could be produced via this electrolysis?

Balance the following half-reaction occurring in basic solution. ​ MnO2(s)→ Mn(OH)2(s)

When an aqueous solution of sodium sulfate is electrolyzed,what are the expected products? Reduction Half-Reaction E° (V) Na+(aq​)+ e¯ Na(s) -2.71 2H2O(l)+ 2e- H2(g)+ 2OH-(aq) -0.83 2H+(aq)+ 2e- H2(g) 0.00 O2(g)+ 4H+(aq)+ 4e- 2H2O(l)1.23 S2O82-(aq)+ 2e- 2SO42-(aq) 2.01

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Given: Hg²⁺(aq)+ 2e^- Hg(s); E° = 0.85 V Li⁺(aq)+ e^- Li(s); E° = -3.04 V Br₂(l)+ 2e^- 2Br^-(aq); E° = 1.07 V Au⁺(aq)+ e^- Au(s); E° = 1.69 V Cl₂(g)+ 2e^- 2Cl^-(aq); E° = 1.36 V Which of the following species is the best reducing agent?

When the following oxidation-reduction reaction in acidic solution is balanced,what is the lowest whole-number coefficient for H⁺,and on which side of the balanced equation should it appear? MnO₄^-(aq)+ I^-(aq)→ Mn²⁺(aq)+ I₂(s)

What is the value of the reaction quotient,Q,for the voltaic cell constructed from the following two half-reactions when the Zn²⁺ concentration is 0.0120 M and the Ag⁺ concentration is 1.27 M?

For the cell reaction 2MnO₄^- (aq)+ 5SO₂(g)+ 2H₂O(l) → 2Mn²⁺(aq)+ 5SO^2-₄ (aq)+ 4H⁺(aq) The standard cell potential is 1.34 V.To determine the cell potential at nonstandard conditions,what is the value that should be used for n in the Nernst equation?

A zinc-copper voltaic cell is represented as follows: Zn(s)| Zn²⁺(1.0 M)|| Cu²⁺(1.0 M)| Cu(s) Which of the following statements is false?

Given: Pb²⁺ (aq)+ 2e¯ Pb(s); Eº = -0.13V What is the standard Gibbs free-energy change for the following reaction? 2Cr(s)+ 3Pb²⁺ (aq)→ 3Pb(s)+ 2Cr³⁺ (aq)

In the electrolysis of an acid solution,oxygen can be produced by the following half-reaction: 2H₂O(l)→ O₂(g)+ 4H⁺(aq)+ 4e^- How many moles of O₂ can be produced from a solution that was electrolyzed for 6.50 h using a current of 5.40 A?

If the cell is initially at standard-state conditions,which of the following statements is true? Zn²⁺(aq)+ 2e^- Zn(s); E° = -0.76 V Cu²⁺(aq)+ 2e^- Cu(s); E° = 0.34 V

How many faradays are required to convert a mole of NO₃^- ions to NH₄⁺ ions?

Consider the following standard reduction potentials: Mg²⁺(aq)+ 2e^- Mg(s); E° = -2.38 V V²⁺(aq)+ 2e^- V(s); E° = -1.18 V Cu²⁺(aq)+ e^- Cu⁺(aq); E° = 0.15 V Which of the following reactions will proceed spontaneously from left to right under standard-state conditions?

Balance the following half-reaction occurring in basic solution. MnO₂(s)→ Mn(OH)₂(s)

When an aqueous solution of sodium sulfate is electrolyzed,what are the expected products? Reduction Half-Reaction E° (V) Na⁺(aq)+ e¯ Na(s) -2.71 2H₂O(l)+ 2e^- H₂(g)+ 2OH^-(aq) -0.83 2H⁺(aq)+ 2e^- H₂(g) 0.00 O₂(g)+ 4H⁺(aq)+ 4e^- 2H₂O(l)1.23 S₂O₈^2-(aq)+ 2e^- 2SO₄^2-(aq) 2.01